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Strength of a weak acid or a weak base d...

Strength of a weak acid or a weak base depends upon its

A

Temperature

B

Nature of solvent

C

Degree of dissociation

D

All the above

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D
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Define pH. pH cannot be calculated directly from the molar concentration of a weak acid or weak base. Why? Derive an equation for the pH of a weak acid.

When a salt reacts with water to form acidic (or ) basic solution the process is called salt hydrolysis. The P^(H) of salt solution can be calculated using the following relation P^(H) =(1)/(2) [P^(k_w) +P^(Ka) + log C ] for salt of weak acid and strong base. P^(H) =(1)/(2) [P^(K_w) -P^(K_a) -log C ] for salt of weak base and strong acid , P^(H) =(1)/(2) [P^(K_w) +P^(K_a) - P^(K_b) ] For a salt of weak acid and weak base where .c. represents the concentration of salt . When a weak acid (or) a weak base is not completly neatralised by strong base (or ) strong acid respectively, then formation of buffer takes places. The P^(H) of buffer solution can be calculated using the following relation P^(H) =P^(Ka) +log "" ((["salt")])/(["Acid "]) , P^(OH) =P^(Kb) +log ""(["salt"])/(["base"]) Answer the following questions using the following data pK_a (CH_3COOH) =4.7447 , pK_b (NH_4OH) =4.7447 , P^(K_W) =14. One mole CH_3 COOH and one mole CH_3 COONa are dissolved in water one litre aqueous solution The P^(H) of the resulting solution will be

When a salt reacts with water to form acidic (or ) basic solution the process is called salt hydrolysis. The P^(H) of salt solution can be calculated using the following relation P^(H) =(1)/(2) [P^(k_w) +P^(Ka) + log C ] for salt of weak acid and strong base. P^(H) =(1)/(2) [P^(K_w) -P^(K_a) -log C ] for salt of weak base and strong acid , P^(H) =(1)/(2) [P^(K_w) +P^(K_a) - P^(K_b) ] For a salt of weak acid and weak base where .c. represents the concentration of salt . When a weak acid (or) a weak base is not completly neatralised by strong base (or ) strong acid respectively, then formation of buffer takes places. The P^(H) of buffer solution can be calculated using the following relation P^(H) =P^(Ka) +log "" ((["salt")])/(["Acid "]) , P^(OH) =P^(Kb) +log ""(["salt"])/(["base"]) Answer the following questions using the following data pK_a (CH_3COOH) =4.7447 , pK_b (NH_4OH) =4.7447 , P^(K_W) =14. 0.001 M NH_4 Cl aqueous solution has P^(H)

The percentage degree of hydrolysis of a salt of weak acid (HA) and weak base (BOH) in its 0.1 M solutions is found to be 10% If the molarity of the solution is 0.05M , the percentage hydrolysis of the salt should be :

Guanidine (I) and its conjugate acid (II) are given below along with urea(III) and its conjugate base (IV) Basic properties of I & II compounds are mainly influenced by resonance and the acidity of the bases depends upon lone pair of electrons. The strongest base of the following is

Guanidine (I) and its conjugate acid (II) are given below along with urea(III) and its conjugate base (IV) Basic properties of I & II compounds are mainly influenced by resonance and the acidity of the bases depends upon lone pair of electrons. The strongest base of the following is

Guanidine (I) and its conjugate acid (II) are given below along with urea(III) and its conjugate base (IV) Basic properties of I & II compounds are mainly influenced by resonance and the acidity of the bases depends upon lone pair of electrons. Urea is mono basic because

AAKASH SERIES-IONIC EQUILIBRIUM -LECTURE SHEET (EXERCISE -II LEVEL -I (MAIN) (Straight Objective Type Questions))
  1. At infinite dilution , the percentage ionisation of both strong and we...

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  2. Which of the following is the best conductor of electricity ?

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  3. Strength of a weak acid or a weak base depends upon its

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  4. The P^(H) of 0.001 M CH(3),COOH is

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  5. Which of the following is relatively stronger acid? K, values are give...

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  6. A monoprotic acid in a 0.1 M solution ionizes to 0.001 % . Its ionizat...

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  7. The hydrogen ion concentration of 0.2 M CH3 COOH which is 4% ionised ...

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  8. pH of a weakacid in 0.1 M solution is 4.3. Which statements are correc...

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  9. Dissociation constant of water at 25^(@) C is

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  10. At any temperature, P^(H) +P^(OH) is equal to

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  11. At any temperature ,the proton concentration of water is

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  12. At certain temperature, the H^(+) ion concentration of water is 4 xx 1...

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  13. At 298 K, the [H(2),O^(+)] of a solution is 2 xx 10^(-9) M. The natur...

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  14. At a given temperature, When an acid is added to water then the value ...

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  15. At 100^(@)C, the P^(H) of pure water is

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  16. At some high temperature, K(w) of water is 10^(-13) Then the P^(H) of ...

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  17. Among the following (a) P^(H) of water decreases with increase i...

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  18. The H^(+) ion concentration of a solution is 4xx10^(-5) M. Then th...

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  19. 0.004 g of NaOH is present in 1L of a solution. The pH of the solut...

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  20. The P^(H) of 0.005 M Ba (OH)(2) is

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